10.4 Real Gases & the Van der Waals Equation | General Chemistry

Chad provides an introduction to Real Gases contrasting them with Ideal Gases. How their behavior differs due to attractive forces and molecular volume is shown and then quantified with the Van der Waals Equation. Sample calculations are performed comparing pressures calculated using the Ideal Gas Law and the Van der Waals equation showing how the difference is often more significant at higher pressures.
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00:00 Lesson Introduction
00:44 Graphs of Compressibility for Real Gases
03:15 The Van der Waals Equation
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[@jenny2665]

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[@skylardean4540]

Chad coming in clutch, once again!

[@ChadsPrep]

Glad the channel is helping you!

[@briantran9211]

Hey Chad, I just calculated the pressure using van der waals through my calculator and got 23.34811 by any chance do you know what I did wrong to get this answer?

[@phonognome6218]

you have to subtract nb from V. you plugged it in your calc wrong.. P=((nrt)/(v-(nb)))-((an^2/(v^2)) should do the trick.

[@jmac5501]

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[@ChadsPrep]

No merch right now, JMAC - maybe someday in the future. Thanks for asking!

[@asmaaali462]

Real gases do not obey perfect gas law exactly are particularly important at high pressure and.........high temperature or low temperature?

[@joshualogronio4772]

low temperature

[@ruoyluos9814]

Low temperature, bcuz gas possessed small kinetic energy which they will move very slowly n become closer With one another, hence IMF become more significant